Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH₃CH₂CH₂COOH (Kₐ=1.54X10⁻⁵), with0.1000 M NaOH solution after the following additions of titrant:(a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 19.00 mL(e) 19.95 mL(f ) 20.00 mL(g) 20.05 mL(h) 25.00 mL

Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH₃CH₂CH₂COOH (Kₐ=1.54X10⁻⁵), with0.1000 M NaOH solution after the following additions of titrant:(a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 19.00 mL(e) 19.95 mL(f ) 20.00 mL(g) 20.05 mL(h) 25.00 mL

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.71PAE: Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’....

See similar textbooks

Related questions

Q: If (HSO, ] = .3 M, what [SO,² ] is needed to make a buffer of pH 2.6?

Q: From their Kb values, which of the following bases would be best for preparing a buffer of pH 9.00:…

A: Basic buffer is a solution of weak base and its salt. Salt is formed by reaction of weak base and…

Q: What masses of acetic acid and sodium acetate are needed to prepare 125 mL of pH=5.00 buffer if the…

A: Number of moles of solute to the volume of solution in liter is known as molarity.

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

A: Answer: When a weak acid is added into water, it furnishes and these free ions conducts the…

Q: What will be the total buffer concentration? What is the pH of a solution contains acetic acid d…

A: The solution which is made by the mixing of a weak acid and its conjugate base or vice verse is know…

Q: A 25mL sample of a 0.15M solution of a weak acid Ka=3.0x10^-6 is titrated ith 0.15M NaOH. What is…

A: Calculate the number of moles of weak acid and the strong base NaOH. The number of moles can be…

Q: the answer) Calculate the pH of a buffer that is 0.158 M HCIO and 0.099 M NaCIO. The K, for HCIO is…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: The acid–base indicator bromcresol green is a weak acid.The yellow acid and blue base forms of the…

A: The acid-base titration is involves the reaction of acid with base to calculate the concentration of…

Q: A. What is the pH of a buffer prepared by adding 0.607 molof the weak acid HA to 0.406 mol of NaA in…

Q: What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10³ ) is added to 100.0 mL of a…

A: Given: Concentration of HOAc in buffer = 0.1000 M Concentration of NaOAc in buffer = 0.1000 M Volume…

Q: You prepare 250.0 mL of a buffer solution containing 0.550mol of acid and 0.450mol of its conjugate…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Calculate the initial [H,O*] in mol/L in the weak acid sample using the initial pH measurement. Show…

A: Initial [H3O+] can be calculated using initial pH of solution of weak acid.

Q: What masses of dimethylamine and dimethylammonium chloride do you need to prepare 3.00 L of pH =…

A: Given, The volume of dimethyl amine and dimethyl ammonium chloride buffer = 3.00L The total…

Q: What is the pH of a buffer solution containing 0.30 M HCOOH(aq) and 0.051 M NaHCOO(aq)? The acid…

A: The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of…

Q: 2. In the pH metric titration of strong and weak acid mixture against strong alkali, generally first…

A: We are given a mixture of strong acid(H+) and weak acid(HA). We titrate the above mixture with a…

Q: IN CASE OF TITRATION OF WEAK ACID IN A NON-AQUEOUS MEDIUM, THE INDICATOR IS USED Choose one answer:…

A: Correct option is D

Q: A laboratory manager wants to prepare 500.00 mL of a buffer with a pH of 4.471 from equimolar…

A: Ka = 1.8 x 10-5 pKa = 4.745 pH of buffer solution = 4.471 Let volume of CH3CO2H required = V ml…

Q: A 24.5 mL sample of 0.249 M methylamine, CH3NH2, is titrated with 0.234 M perchloric acid.At the…

A: The acid-base reaction between methylamine (CH3NH2) and perchloric acid (HClO4) can be written asThe…

Q: When 50mL of 0.10 M HOAc is titrated with 25mL of 0.1O M NaOH, the pH is

A: Given, Volume of acetic acid = 50mL. Concentration of acetic acid = 0.10M. Volume of NaOH = 25mL.…

Q: A 47.1 mL sample of a 0.548 M aqueous acetic acid solution is titrated with a 0.426 M aqueous sodium…

A: The balanced chemical equation is: CH3COOH (aq) + NaOH (aq) ---> CH3COONa (aq) + H2O (l)

Q: How many milllilitres of HCl should you add to 250.00mL of 13.4 x 105 ppm sodium maleate to produce…

A: We have to find the volume of HCl such that we get pH = 3.37 Given 250.00mL of 13.4 x 10⁵ ppm…

Q: A laboratory manager wants to prepare 250.00 mL of a buffer with a pH of 3.514 from equimolar…

A: The given data contains, Volume = 250 ml. pH = 3.514 Ka of HCOOH=1.8×10-4

Q: Can someone explain part B for me I don't understand why [HX]>[X-].

A: Given information: The pKa for weak acid = 4.5 The pH of the buffer solution = 4.3

Q: 16 The pH of blood plasma is 7.40. Assuming the prin- cipal buffer system is HCO,/H,CO3, calculate…

Q: Calculate the ratio of [Ca2+ ] to [Fe2+ ] in a lake in whichthe water is in equilibrium with…

A: Solubility product constant for CaCO3 is 4.5x10-9. Solubility product constant for FeCO3 is…

Q: The Ka expression for the H, PO,/HPO;- buffer is given Ionic strength (µ, M) 0.005 0.010 0.050 0.10…

Q: A buffer is prepared by adding 35 mL of 0.100 M hypochlorous acid, HOCl, to 65 mL of 0.300 M…

Q: Raferences) hat is the pH change when 18.5 ml of 0.137 M NaOH is added to 64.8 ml of a buffer…

Q: The director of a chemical analysis laboratory is told to expect a large number of samples for which…

A: Fajans method is an analytical method for titrimetric determination of halogen in a compound. The…

Q: A laboratory manager wants to prepare 250.00 mL of a buffer with a pH of 8.576 from equimolar…

A: Solution - According to the question - Given - Total volume = 250.00 mL pH = 8.570 Ka = 2.000e-9…

Q: A 26.2 mL sample of 0.253 M trimethylamine, (CH3)3N, is titrated with 0.306 M hydroiodic acid. At…

A: Given data : 1. 26.2 mL sample of 0.253 M trimethylamine, (CH3)3N 2 . 0.306 M hydroiodic acid. To…

Q: (3) How will you prepare 500 ml of 0.750 M citrate buffer with pH of 4.25 from solid citric acid…

A: Molarity of buffer to be prepared [AH] = 0.750 M Volume of buffer solution = 500 ml pH of buffer…

Q: A 15.00 ml aliquot of a 0.75 M solution of a weak acid (K, = 1.00E-05 at 25°C) is titrated with…

Q: [20] ml of [4] M HC2H3O2 is titrated with 2.25 M sodium hydroxide. Ka for HC2H3O2 is 1.8 x 10-5 d.…

A: Given: Concentration of HC2H3O2 (assuming it HA) = 4 M The volume of HA taken = 20 mL And the…

Q: A 25.5 mL sample of 0.362 M triethylamine, (C2H5)3N, is titrated with 0.285 M hydroiodic acid.…

A: Given data,Molarity of triethylamine=0.362MVolume of triethylamine=25.5mL=0.0255LMolarity of…

Q: Calculate the pH of the following buffers:a) A solution containing 0.425 molar benzoic acid and…

A: Calculate the value of pKa: Ka of benzoic acid is 6.50 × 10-5.

Q: A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The…

A: We have to predict the molar mass, effect on molar mass.

Q: What is the pH change when 28.8 mL of 0.0540 M NaOH is added to 70.1 mL of a buffer solution…

Q: The Ka expression for the H,PO,/HPO;- buffer is given by the equation Ionic strength (µ, M) 0.005…

A: The Ka for the H2PO4-/HPO42- buffer is given by the equation: What is the pH of a 3:4 mixture of ...

Q: A 50.00-mL sample of a 0.250 M solution of butyric acid, HB, (K = 1.5 x 10 ) is titrated with 0.125…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: A 100 ml of 0.100 M phosphate buffer solution with a pH of 8.10 is to be prepared by adding 1.00 M…

A: The required pH of the buffer is 8.10, which is closest to the pKa2 value. H2PO4(aq) ⇌ HPO4-(aq) +…

Q: 4. A solution was prepared by dissolving 0.541 g of benzoic acid (HC,HSCOO) in 100 mL of water. The…

Q: Which of the following will raise the pH of a weak acid HA in aqueous solution? I. addition of HNO3…

A: (I) HNO3 is a strong acid and thus decreases the pH of the solution. Therefore, pH won’t increase on…

Q: 2. In titration experiment at 25°C, a total of 30 mL of 0.1 M NaOH was added dropwise to conical…

A: The question is based on the concept of titrations. We are titrating a strong acid and strong base.…

Q: A student needs to prepare a buffer made from HNO2 and NaNO2 with pH 3.655. If Ka for HNO2 is 4.50 x…

A: Given : The solution is a buffer solution with HNO2 acid and its conjugate base salt NaNO2. pH of…

Q: How many grams of solid calcium cyanide, Ca(CN)₂ must be added to 200.0 ml of 0.370M hydrocyanic…

A: Molarity of HCN = 0.370 M pH = 9.20

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2,M(OH)2, is mixed with pure water.…

A: Given that,PH of the solution = 10.28Ksp =?You know thatPH + POH = 14

Q: 3. What is the pH of the carbonic acid if 20.00 mL of 0.0500 M H,CO3 is titrated with (a) 0.00 mL…

A: Since, you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Q: Consider the titration of 15.75 mL of 0.549 M potassium propanoate, CH3CH;CO,K, with 0.207 M HNO3.…

A: Given : Concentration of CH3CH2CO2K = 0.549 M Volume of CH3CH2CO2K solution = 15.75 mL = 0.01575 L…

Q: 7. A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in…

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid:(a) 6.00 mL (b) 29.80 mL (c) 35.00 mL
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base: (a) 28.00 mL (b) 39.50 mL (c) 52.00 mL
Find the pH during the titration of 20.00 mL of 0.1000 Mtri-ethylamine, (CH₃CH₂)₃N (K(b)=5.2X10⁻⁴), with 0.1000 M HCl solution after the following additions of titrant:(a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 19.00 mL(e) 19.95 mL(f ) 20.00 mL(g) 20.05 mL(h) 25.00 mL
Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid: (a) 0 mL (b) 18.00 mL (c) 30.00 mL (d) 35.10 mL
A 76.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M RbOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.1 mL pH = 3.32 (d) 39.9 mL pH = 9.58 X X (b) 37.2 mL pH = 4.79 (e) 69.5 mL pH = 10.79 X X (c) 38.0 mL pH = 7
A buffer is made with sodium acetate (CH3COONa) andacetic acid (CH3COOH); the Ka for acetic acid is 1.80 x 10-5.The pH of the buffer is 3.98. What is the ratio of the equilibriumconcentration of sodium acetate to that of acetic acid?(a) -0.760 (b) 0.174 (c) 0.840 (d) 5.75 (e) Not enough informationis given to answer this question.
Calculate the pH during the titration of 40.00 mL of 0.1000 M propanoic acid (HPr; Ka = 1.3x10-5) after each of the following additions of 0.1000 M NaOH:(a) 0.00 mL (b) 30.00 mL (c) 40.00 mL (d) 50.00 mL
(7) Calculate the pH of each of the following solutions: (a) 0.1000M Propanoic acid( HC H O,,K=1.3x105) (b) 0.1000M sodium propanoate (Na C HỎ) (c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂ 3 5 52 (d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above. (e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.
Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base:(a) 0 mL(b) 25.00 mL(c) 39.00 mL(d) 39.90 mL(e) 40.00 mL(f ) 40.10 mL(g) 50.00 mL Use the values obtained to sketch a curveof [H₃O⁺] vs. mL of added titrant. Are there advantages or dis-advantages to viewing the results in this form? Explain.
Consider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d please
A 93.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M LIOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.4 mL pH = 2.57 (d) 47.4 mL pH = X X (b) 44.2 mL pH = (e) 78.1 mL pH = X X (c) 46.5 mL pH = X
Consider the titration of 36.0 mL of 0.123 M ammonia with 0.0766 M HCl. (See the Acid-Base Table attached.) (a) How many mL of HCl are required to reach the equivalence point?57.8 mL(b) What is the pH at the equivalence point? 5.29(c) What is the pH of the solution after the addition of 17.2 mL of acid? (d) What is the pH of the solution after the addition of 84.3 mL of acid? (only need help witn c and d)